At 300 K , the $E_{\text {cell }}^{\ominus}$ of

$$ A(s)+B^{2+}(a q) \rightleftharpoons A^{2+}(a q)+B(s) $$

is 1.0 V . If $\Delta_r S^\theta$ of this reaction is $100 \mathrm{JK}^{-1}$. What is $\Delta_r H^{\ominus}$ (in $\mathrm{kJ} \mathrm{mol}^{-1}$ ) of this reaction?

$$ \left(\mathrm{F}=96500 \mathrm{C} \mathrm{~mol}^{-1}\right) $$

Consider the cell reaction at 300 K .

$$ A(s)+B^{2+}(a q) \rightleftharpoons A^{2+}(a q)+B(s) $$

Its $E^{\ominus}$ is 1.0 V . The $\Delta_r H^{\ominus}$ of the reaction is $-163 \mathrm{kJmol}^{-1}$.

What is $\Delta_r s^{\ominus}$ (in $\mathrm{JK}^{-1}$ ) of the reaction?

$$ \left(F=96500 \mathrm{C} \mathrm{~mol}^{-1}\right) $$

In which of the following Galvanic cells emf is maximum?

(Given, $E_{\mathrm{Mg}^{2+} \mid \mathrm{Mg}}^{\circ}=-2.36 \mathrm{~V}$

and $E_{\mathrm{Cl}_2 \mid 2 \mathrm{Cl}^{-}}^{\circ}=+136 \mathrm{~V}$ )

Consider the following standard electrode potentials ( $E^{\circ}$ in volts) in aqueous solution.

$$ \begin{array}{|c|c|c|} \hline \text { Element } & M^{3+} / M & M^{+} / M \\ \hline \mathrm{Al} & -1.66 & +0.55 \\ \hline \mathrm{TI} & +1.26 & -0.34 \\ \hline \end{array} $$

Based on this data. which of the following statements is correct?